1. A solution contains 28% phosphoric acid by mass. This means that: A.)100 ml of this solution contains 28 g of phosphoric acid B. I ml of this solution contains 28 g of phosphoric acid C. 1 L of this solution contains 28 mL of phosphoric acid
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- Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). then transfer FeII to 100 ml flask makeup to the mark with water. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL.Beaker 0.00200 M Fe(NO3)3, mL 0.00200 M NaSCN, mL total volume, mL 1 3.000 2.000 10.00 2 3.000 3.000 10.00 3 3.000 4.000 10.00 4 3.000 5.000 10.00 5 (blank) 3.000 0.000 10.00 In Solutions 1-4 you are adding successively larger volumes of 0.00200M SCN- to the Fe3+ solution and diluting to 10.00 ml. Calculate the final diluted molarity of SCN- in solution #1 Your answer should have 3 sig figs =In this station, you will find a sample of table salt; the chemical formula of table salt is NaCl. Using the balance, weigh out 6.00 g of NaCl and dissolve in 50 mL of deionized (d.i.) water. Once com-pletely dissolved, add additional d.i. water to make the final volume of solution 100.0 mL. What is the mass percent NaCl in the solution? What is the molarity of the solution
- and Employees CH STATE GE 90 ENDULERSE IS FOREVER "ON-Tame Name Jodi Rayal Molarity = wt. x1000 3. Calculate the massof Potassium hydrogen phthalate (KHP) to prepare a 250.0 mL solution of 0.1000 M KHP solution. Mol ut. x Voluse the 2500×1000 204.22250 mass Initial Buret Reading Final Buret Reading Vol NaOH Added Moles of NaOH Moles of HCI Volume of unknown HCI solution Concentration of HCI Average concentration of HCI of KHP = 5.11g 4. Complete the table below for the following neutralization reaction of an unknown concentration of hydrochloric acid with 0.100 M sodium hydroxide: Mu spate solution Trial 1 0 11.15 го data and calculate the concentration 15 Trial 2 11.15 22.15 Trial 3 22.15 33.25 abyh 067 LANDINUKASHU TROWTHCENTISSATE ARAD Ma That par މއކނި REMURNAR MISAMARALISERDRY TileIn the standardization of HCl using pure anhydrous sodium carbonate as the primarystandard for methyl orange as an indicator, 1.0 mL HCl was found to be equivalent to 0.05gof sodium carbonate (MW =106). The normality of HCl is:How would I solve Problem 4? I have the excel graph as provided. Need to get the %Mn I have some small idea but think is wrong... would be... %Mn = 500mL * 1molMn/ g MnO4 * 1molMn/1molMnO4- * gMn/1molMn * 100%/SampleMassg
- Come up with a dilution scheme starting from 1000 μg/mL Mn stock solution so that the concentration of permanganate in the solutions just prior to measurement (after Step B.6.) are: 7.5, 15.0, 22.5, 30.0 and 37.5 μg/mL MnO4-. Carefully read the units!50.00 cm3 of a 1.5784 mol.dm-3 solution of potassium hydroxide is transferred to an empty 700.00 cm3 volumetric flask. This flask is made up to the mark with distilled water and then shaken well. The concentration of the potassium hydroxide in this second flask is:1.) Use the line of best ! Tables: Data Port 1. Synthesis of Asprin \table[[Mass of galicylic Acid used 2.024gt to calculate the concentration of the salicylic Acid in your asprin saple solution (in 50.0 ml volumettic flask) 2.) Use M1V1 = M2V2 to determine the concentration of salicylic acid in your 100.0 mL solution before dilutuon to 50.0mL for analysis. 3.) Determine the mass of salicylic acid present in the 4g sample of synthesized asprin tht was dissolved in the 100.0ml, volumetric flask 4.) Determine the percent of salicylic acid and percent asprin in the 4g sample of synthesized asprin7 5.) Calculate the theoretical yelld of asprin for your synthesis reaction. Assume that the salicylic acid used in the salicylic used in the synthesis reaction is the limiting reactant. 6. Determine the percent yild of the asprin for your synthesis. For the 1st cacization i got 1.340x10^-4 M C7H603 For the 2nd calculation i got M167x10^-5 Please check my calculations and explain the remaining
- A 25mL volumetric pipet is used to deliver a sample of the stock solution marked “0.6000M X2SO4” into a 100mL volumetric flask. Distilled water is added to the flask until it is about 3/4thfull, the solution is mixed well, then more water is added to fill it up to the calibration mark, then it is mixed again. Calculate the concentration of X+ion in the dilute solution made above.I am allowed to work with someone I just don’t understand this Using the Volumetric Pipet Data from Part C calculate the: 7. Mass (g) and density (g / m L) of the first addition of saline25 ppm of CaCO3 was found in the water sample obtained on the lake in the nearby town.Calculate the moles of CaCO3 having a molar mass of 100.09 g/mol in 10 liters of water samplesolution having a density of 997 kg/m3. (Ans.: 24.95 moles CaCO3)